2. a 10.00ml diluted chloride sample required 13.89 ml of 0.02014 M AgNo3 to reach the fajans endpoint. a. how many moles of Cl- ion were present in the sample b. what was the concentration of chloride in the diluted solution
2. a 10.00ml diluted chloride sample required 13.89 ml of 0.02014 M AgNo3 to reach the fajans endpoint. a. how many moles of Cl- ion were present in the sample b. what was the concentration of chloride in the diluted solution
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2. a 10.00ml diluted chloride sample required 13.89 ml of 0.02014 M AgNo3 to reach the fajans endpoint.
a. how many moles of Cl- ion were present in the sample
b. what was the concentration of chloride in the diluted solution?
![### Experiment 7: Analysis of an Unknown Chloride
**Advance Study Assignment**
1. **A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802 M, and 0.02788 M.**
- a. **What is the mean concentration?**
- \_\_\_\_\_\_\_\_\_\_\_ M
- b. **What is the standard deviation of these results?**
- \_\_\_\_\_\_\_\_\_\_\_ M
2. **A 10.00 mL diluted chloride sample required 13.89 mL of 0.02014 M AgNO₃ to reach the Fajans endpoint.**
- a. **How many moles of Cl⁻ ion were present in the sample? (Use Eqs. 2 and 3.)**
- Calculation:
- \( \text{Moles of Ag}^+ = \text{Moles of AgNO}_3 \)
\[ \text{Moles of Ag}^+ = 0.02014 M \times 0.01389 L \]
\[ = 0.00028 \text{ moles} \]
- \_\_\_\_\_\_\_\_\_\_\_ moles Cl⁻
- b. **What was the concentration of chloride in the diluted solution?**
- Calculation:
\[ M_2 = \frac{0.02014 M \times 13.89 \text{ mL}}{10.00 \text{ mL}} \]
\[ = \frac{0.28}{10.00} \]
\[ = 0.028 \text{ M} \]
- \_\_\_\_\_\_\_\_\_\_\_ M
3. **How would the following errors affect the concentration of Cl⁻ obtained in Question 2b? Give your reasoning in each case.**
- a. **The student read the molarity of AgNO₃ as 0.02104 M instead of 0.02014 M.**
- b. **The student was past the endpoint of the titration when he took the final buret reading.**
**Explanation of Graphs or Diagrams (if any)**:
- There are no graphs or diagrams](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdec5afcc-1b1f-4d8a-a91d-78428b1875fd%2F65897d85-4a5c-4f9d-a5b0-53d9dfa14ec6%2Fvq841q9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Experiment 7: Analysis of an Unknown Chloride
**Advance Study Assignment**
1. **A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802 M, and 0.02788 M.**
- a. **What is the mean concentration?**
- \_\_\_\_\_\_\_\_\_\_\_ M
- b. **What is the standard deviation of these results?**
- \_\_\_\_\_\_\_\_\_\_\_ M
2. **A 10.00 mL diluted chloride sample required 13.89 mL of 0.02014 M AgNO₃ to reach the Fajans endpoint.**
- a. **How many moles of Cl⁻ ion were present in the sample? (Use Eqs. 2 and 3.)**
- Calculation:
- \( \text{Moles of Ag}^+ = \text{Moles of AgNO}_3 \)
\[ \text{Moles of Ag}^+ = 0.02014 M \times 0.01389 L \]
\[ = 0.00028 \text{ moles} \]
- \_\_\_\_\_\_\_\_\_\_\_ moles Cl⁻
- b. **What was the concentration of chloride in the diluted solution?**
- Calculation:
\[ M_2 = \frac{0.02014 M \times 13.89 \text{ mL}}{10.00 \text{ mL}} \]
\[ = \frac{0.28}{10.00} \]
\[ = 0.028 \text{ M} \]
- \_\_\_\_\_\_\_\_\_\_\_ M
3. **How would the following errors affect the concentration of Cl⁻ obtained in Question 2b? Give your reasoning in each case.**
- a. **The student read the molarity of AgNO₃ as 0.02104 M instead of 0.02014 M.**
- b. **The student was past the endpoint of the titration when he took the final buret reading.**
**Explanation of Graphs or Diagrams (if any)**:
- There are no graphs or diagrams
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